Orbital Hybridization 2

A carbon atom forming 3 equivalent bonds and a double bond, uses sp2 hybrid orbitals.

A carbon atom forming 1 bond with a terminal carbon, 1 with adjacent carbon and 2 more bonds with the terminal carbon uses sp hybrid orbitals.

A covalent bond formed by head-on or end-to-end overlap of atomic orbitals.

A covalent bond formed by side-to-side overlap of atomic orbitals.

In the given options for this question - CF4 - tetrahedral, BeBr2 - linear, H2O - tetrahedral, NH3 - tetrahedral, PF3 - octahedral, only PF3 has an incorrect match

NF3 - trigonal planar is incorrect. Other listed molecules have correct matches.

A molecule with an arrangement of atoms along a straight line, like in Carbon Dioxide (CO2).

Used by the carbon atom in forming 4 single bonds, as in CF4 molecule

Boron trifluoride (BF3) has sp2 hybridization, meaning the boron atom uses 2 p orbitals and 1 s orbital to form 3 equivalent hybrid orbitals.

Different numbers of electron orbitals around an atom result in unique hybridisation and shapes.

Chloroform (CHCl3) has a central carbon atom with four equivalent bonds, which results in sp3 hybridization.

Different arrangements of bonds around carbon atoms influence the hybridization, directly impacting molecular shapes.

The number of bonds formed by a central atom determines its hybridization.

The octet rule, which predicts that atoms gain or lose electrons to achieve a stable outer shell with eight electrons, works well with p orbitals but not with d orbitals.

In sp3d hybridization, one s, three p and one d atomic orbital on a central atom combine to form five equivalent hybrid orbitals. This allows the atom to form five bonds, like in PCl5.

PCl5 has a trigonal bipyramidal shape. There are three equatorial P-Cl bonds in the same plane at 120° angles, and two axial P-Cl bonds perpendicular to this plane at 90° angles.

In sp3d2 hybridization, one s, three p and two d atomic orbitals on a central atom combine to form six equivalent hybrid orbitals. This allows the atom to form six bonds, like in SF6.

SF6 has an octahedral shape with bond angles of 90° between the six hybrid orbitals.

Boron has only three valence electrons and needs two more to achieve the stable octet configuration. This electron deficiency makes BF3 an electrophile, meaning it seeks electrons to form bonds.

A molecule with sp3 hybridization will have a tetrahedral shape with bond angles of approximately 109.5 degrees.

A molecule with sp2 hybridization will have a trigonal planar shape, with bond angles of 120 degrees.

The number of bonds a central atom forms directly influences its hybridization and ultimately the shape of the molecule.

The number of bonds an atom forms and the presence of lone pairs contribute to determining hybridization.

PCl5 has a trigonal bipyramidal shape. There are three equatorial P-Cl bonds in the same plane at 120° angles, and two axial P-Cl bonds perpendicular to this plane at 90° angles.

The trigonal planar geometry of BF3, with 120° bond angles, arises from its sp2 hybridization. This geometry leaves the boron atom with an empty p orbital, which can readily accept electrons from other molecules, making BF3 an electrophile.

A molecule in its ground state is at its lowest energy level, with its electrons occupying the lowest possible energy orbitals. This is the most stable configuration.

A carbon atom forming 3 equivalent bonds and a double bond utilizes sp2 hybrid orbitals. This results in a trigonal planar geometry around the carbon atom with bond angles close to 120 degrees.

A carbon atom forming one sigma bond with a terminal carbon, one sigma bond with an adjacent carbon, and two additional sigma bonds with the terminal carbon utilizes sp hybrid orbitals. This leads to a linear geometry.

PF3 has a tetrahedral electron geometry but a trigonal pyramidal molecular geometry due to the lone pair on the phosphorus atom which repels the bonding pairs.

NF3 has a trigonal pyramidal molecular geometry due to the lone pair on the nitrogen atom, which repels the fluorine atoms.

A molecule with an arrangement of atoms along a straight line. This arrangement arises from the sp hybridization of the central atom.

The carbon atom in CF4 utilizes sp3 hybrid orbitals to form four equivalent single bonds to the fluorine atoms, giving it a tetrahedral geometry.